If 29.8 ml of the H_3PO_4 (phosphoric acid) reacts with 35.0 mL of 5.00 M KOH, what is the...


If 29.8 ml of the {eq}H_3PO_4 {/eq} (phosphoric acid) reacts with 35.0 mL of 5.00 M KOH, what is the molarity of the acid?

{eq}H_3PO_4 + 3KOH \rightleftharpoons K_3PO_4 + 3H_2O {/eq}

Equivalence Point:

In an acid-base titration experiment you begin with an acid/base analyte of unknown concentration in a flask. To this flask is slowly added a standardized base/acid titrant from a burette. Eventually enough of the titrant is added that it just fully neutralizes the analyte in the flask. At this point both reactants are fully consumed and only the products remain. This is known as the equivalence point of an acid-base titration. Using the moles of your standardized titrant at this point you can find the moles of your unknown analyte.

Answer and Explanation: 1

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Phosphoric acid is a triprotic acid. The 1:3 molar acid-base reaction of phosphoric acid with KOH is written as:

{eq}H_3PO_4 + 3KOH \rightarrow...

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Equivalence Point: Definition & Calculation


Chapter 12 / Lesson 11

Learn about equivalence point and end point in titrations. Examine how to find equivalence points in a variety of ways, and discover the steps to do so.

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